Standard electrode potential of three metals X, Y and Z are -1.2 V, +0.5 V and -3.0 V respectively. The reducing power of these metals will be: 

1.	Y > X > Z	2.	Z > X > Y
3.	X > Y > Z	4.	Y > Z > X

For a cell involving one electron ${\mathrm{E}}_{\mathrm{cell}}^{⊝}=0.\mathrm{59 }\mathrm{V}$ at 298 K.
The equilibrium constant for the cell reaction is :
\(\mathrm{[Given~ that~ \frac {2.303 ~RT}{F} = 0.059 ~V~ at~ T = 298 K]}\)

1. $1.0\times {10}^{30}$

2. $1.0\times {10}^2$

3. $1.0\times {10}^5$

4. $1.0\times {10}^{10}$

Given that
I₂ + 2e¯ $\to$ 2I¯; E° = 0.54V
Br₂ + 2e¯ $\to$ 2Br¯; E° = 1.09V

Predict which of the following is true?

The cell potential will be:

The weight of silver (at.wt. = 108) displaced by a quantity of electricity which displaces 5600 mL of O₂ at STP will be:

1. 5.4 g

2. 10.8 g

3. 54.0 g

4. 108.0 g

When 0.1 mol MnO₄^2– is oxidized, the quantity of electricity required to completely oxidise MnO₄^2– to MnO₄^– is:

1. 96500 C

2. 2 × 96500 C

3. 9650 C

4. 96.50 C

The pressure of H₂ required to make the potential of H₂ - electrode zero in pure water at 298 K is:

The number of electrons delivered at the cathode during electrolysis by a current of 1 ampere in 60 seconds is:

(Charge on electron = 1.60 × 10^–19 C)

1.  $6\times {10}^{23}$

2.  $6\times {10}^{20}$

3.  $3.75\times {10}^{20}$

4.  $7.48\times {10}^{20}$